Trihalomethane
In chemistry, trihalomethanes (THMs) are chemical compounds in which three of the four hydrogen atoms of methane (Template:Chem2) are replaced by halogen atoms. Trihalomethanes with all the same halogen atoms are called haloforms. Many trihalomethanes find uses in industry as solvents or refrigerants. Some THMs are also environmental pollutants, and a few are considered carcinogenic.
Table of common trihalomethanes
| Molecular
formula |
IUPAC name | CAS registry number | Common name | Other names | Molecule |
|---|---|---|---|---|---|
| CHF3 | trifluoromethane | 75-46-7 | fluoroform | Freon 23, R-23, HFC-23 | 
|
| CHClF2 | chlorodifluoromethane | 75-45-6 | chlorodifluoromethane | R-22, HCFC-22 | 
|
| CHCl3 | trichloromethane | 67-66-3 | chloroform | R-20, methyl trichloride | 
|
| CHBrCl2 | bromodichloromethane | 75-27-4 | bromodichloromethane | dichlorobromomethane, BDCM | 
|
| CHBr2Cl | dibromochloromethane | 124-48-1 | dibromochloromethane | chlorodibromomethane, CDBM | 
|
| CHBr3 | tribromomethane | 75-25-2 | bromoform | methyl tribromide | 
|
| CHI3 | triiodomethane | 75-47-8 | iodoform | methyl triiodide | 
|
Industrial uses
Only chloroform has significant applications of the haloforms. In the predominant application, chloroform is required for the production of tetrafluoroethylene (TFE), precursor to teflon.[1] Chloroform is fluorinated by reaction with hydrogen fluoride to produce chlorodifluoromethane (R-22). Pyrolysis of chlorodifluoromethane (at 550-750 °C) yields TFE, with difluorocarbene as an intermediate.
Refrigerants and solvents
Trihalomethanes released to the environment break down faster than chlorofluorocarbons (CFCs), thereby doing much less damage to the ozone layer. Trifluoromethane and chlorodifluoromethane are both used as refrigerants. Chlorodifluoromethane is a refrigerant HCFC, or hydrochlorofluorocarbon, while fluoroform is an HFC, or hydrofluorocarbon. Fluoroform is not ozone depleting.
Chloroform is a common solvent in organic chemistry.
Occurrence and production
The total global flux of chloroform through the environment is approximately Template:Val tonnes per year,[2] and about 90% of emissions are natural in origin. Many kinds of seaweed produce chloroform, and fungi are believed to produce chloroform in soil.[3]
Most of the Template:Nowrapspecifically, chloroform (Template:Chem2), bromoform (Template:Chem2), and iodoform Template:Nowrapare easy to prepare through the haloform reaction, although this method does not lend itself to bulk syntheses. (Fluoroform (Template:Chem2) cannot be prepared in this manner.)
Chloroform is produced by heating mixtures of methane or methyl chloride with chlorine. Dichloromethane is a coproduct.[4]
Bromochlorofluoromethane is one of the simplest possible stable chiral compounds, and is used for studies.
Regulation
Trihalomethanes were the subject of the first drinking water regulations issued after passage of the U.S. Safe Drinking Water Act in 1974.[5]
The EPA limits the total concentration of the four chief constituents (chloroform, bromoform, bromodichloromethane, and dibromochloromethane), referred to as total trihalomethanes (TTHM), to 80 parts per billion in treated water.[6]
Traces of chloroform are produced in swimming pools.[7][8][9][10]
References
External links
- National Pollutant Inventory - Chloroform and trichloromethane
- How Ozone Technology Reduces Disinfection Byproducts
- EPA - Trihalomethanes in Drinking Water: Sampling, Analysis, Monitoring and Compliance (August 1983)
Template:Halomethanes Template:Authority control
- ↑ Template:Cite journal
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- ↑ EPA Alumni Association: Senior EPA officials discuss early implementation of the Safe Drinking Water Act of 1974, Video, Transcript (see pages 12-13).
- ↑ Template:Cite web
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